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Chapter 13: Q21E (page 752)

Which of the systems described in Exercise 13.15 give homogeneous equilibria? Which give heterogeneous equilibria?

(a) \(C{H_4}(g) + C{l_2}\rightleftharpoons C{H_3}CI(g) + HCI(g)\)

(b)\({N_2}(g) + {O_2}(g)\rightleftharpoons 2NO(g)\)

(c)\(2S{O_2}(\;g) + {O_2}(\;g)\rightleftharpoons 2S{O_3}(\;g)\)

(d)\(BaS{O_3}(s)\rightleftharpoons BaO(s) + S{O_2}(g)\)

(e) \({P_4}(g) + 5{O_2}(g)\rightleftharpoons{P_4}{O_{10}}(s)\)

(f)\(B{r_2}(\;g)\rightleftharpoons 2Br(g)\)

(g) \(C{H_4}(g) + 2{O_2}(g)\rightleftharpoons C{O_2}(g) + 2{H_2}O(l)\)

(h) \(CuS{O_4} \times 5{H_2}O(s)\rightleftharpoons CuS{O_4}(s) + 5{H_2}O(g)\)

Short Answer

Expert verified
  1. The system is Homogenous.
  2. The system is Homogenous.
  3. The system is Homogenous.
  4. The system is Heterogenous.
  5. The system is Heterogenous.
  6. The system is Homogenous.
  7. The system is Heterogenous.
  8. The system is Heterogenous.

Step by step solution

01

Definition of equilibria

Heterogeneous equilibria is obtained when reactants and products are in separate phases in a chemical reaction, while homogeneous equilibria is obtained when they are in the same phase.

02

Find the system of equilibria for part (a)

a.

The given system is:

\(C{H_4}(g) + C{l_2}\rightleftharpoons C{H_3}CI(g) + HCI(g)\)

Both reactant and product are in same phase, i.e. in the gaseous phase. So, the system is homogenous equilibria.

03

Determine the system of equilibriafor part (b)

b. The given system is:

\({N_2}(g) + {O_2}(g)\rightleftharpoons 2NO(g)\)

Here both reactant and product are in same phase, i.e. in the gaseous phase. So, the system is homogenous equilibria.

04

Detect the system of equilibriafor part (c)

c.

The given system is:

\(2{\rm{S}}{{\rm{O}}_2}(\;{\rm{g}}) + {{\rm{O}}_2}(\;{\rm{g}}) \to 2{\rm{S}}{{\rm{O}}_3}(\;{\rm{g}})\)

Both reactant and product are in same phase, i.e. in the gaseous phase. So, the system is homogenous equilibria.

05

Discover the system of equilibriafor part (d)

d.

The given system is:

\(BaS{O_3}(s)\rightleftharpoons BaO(s) + S{O_2}(g)\)

The phases of reactant and product are different, i.e. solid and gas. So, the system is in heterogeneous equilibrium.

06

Determine the system of equilibriafor part (e)

e.

The given system is:

\({{\rm{P}}_4}(\;{\rm{g}}) + 5{{\rm{O}}_2}(\;{\rm{g}})\rightleftharpoons{{\rm{P}}_4}{{\rm{O}}_{10}}(\;{\rm{S}})\)

The phases of reactant and product are different, i.e. solid and gas. So, the system is in heterogeneous equilibrium.

07

Detect the system of equilibriafor part (f)

f.

The given system is:

\({\rm{B}}{{\rm{r}}_2}(\;{\rm{g}})\rightleftharpoons 2{\rm{Br}}({\rm{g}})\)

Both reactant and product are in same phase, i.e. in the gaseous phase. So, this will give homogenous equilibria.

08

Find the system of equilibriafor part (g)

g.

The given system is as follows:

\({\rm{C}}{{\rm{H}}_4}(\;{\rm{g}}) + 2{{\rm{O}}_2}(\;{\rm{g}})\rightleftharpoons{\rm{C}}{{\rm{O}}_2}(\;{\rm{g}}) + {{\rm{H}}_2}{\rm{O}}({\rm{l}})\)

The phases of reactant and product are different, i.e. solid and gas. So, the system is in heterogeneous equilibrium.

09

Discover the system of equilibriafor part (h)

h.

The given system is:

\({\rm{CuS}}{{\rm{O}}_4}.5{{\rm{H}}_2}{\rm{O}}({\rm{s}})\rightleftharpoons {\rm{CuS}}{{\rm{O}}_4}(\;{\rm{s}}) + 5{{\rm{H}}_2}{\rm{O}}({\rm{l}})\)

The phases of reactant and product are different, i.e. solid and gas. So, the system is in heterogeneous equilibrium.

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Most popular questions from this chapter

Question: Consider the reaction between \({{\rm{H}}_2}\)and \({{\rm{O}}_2}\)at 100 K\({K_P} = \frac{{{{\left( {{P_{{{\rm{H}}_2}{\rm{O}}}}} \right)}^2}}}{{\left( {{P_{{{\rm{O}}_2}}}} \right){{\left( {{P_{{{\rm{H}}_2}}}} \right)}^2}}} = 1.33 \times {10^{20}}\)

If 0.500 atm of H2 and 0.500 atm of O2are allowed to come to equilibrium at this temperature, what are the partial pressures of the components?

What are all concentrations after a mixture that contains \(\left[ {{{\bf{H}}_{\bf{2}}}{\bf{O}}} \right] = {\bf{1}}.{\bf{00Mand}}\left[ {{\bf{C}}{{\bf{l}}_{\bf{2}}}{\bf{O}}} \right] = {\bf{1}}.{\bf{00M}}\) comes to equilibrium at \({\bf{25}}^\circ {\bf{C}}\)?

\({{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}(g) + {\mathbf{C}}{{\mathbf{l}}_{\mathbf{2}}}{\mathbf{O}}(g) \rightleftharpoons {\mathbf{2HOCl}}(g);\;{\mathbf{Kc}} = {\mathbf{0}}.{\mathbf{0900}}\)

Carbon reacts with water vapor at elevated temperatures

\(C(s) + {H_2}O(g) \rightleftharpoons CO(g) + {H_2}(g)\)

\({K_c} = 0.2at100{0^o}C\)

What is the concentration of CO in an equilibrium mixture with \(\left[ {{H_2}O} \right] = 0.500M\)at \(100{0^0}C\)?

Write the mathematical expression for the reaction quotient\({Q_C}\), for each of the following reactions:

(a) \(C{H_4}(g) + C{l_2} \rightleftharpoons C{H_3}CI(g) + HCI(g)\)

(b) \({N_2}(g) + {O_2}(g) \rightleftharpoons 2NO(g)\)

(c) \(2S{O_2}(\;g) + {O_2}(\;g)\rightleftharpoons 2S{O_3}(\;g)\)

(d) \(BaS{O_3}(s)\rightleftharpoons BaO(s) + S{O_2}(g)\)

(e) \({P_4}(g) + 5{O_2}(g)\rightleftharpoons {P_4}{O_{10}}(s)\)

(f) \(B{r_2}(\;g)\rightleftharpoons 2Br(g)\)

(g) \(C{H_4}(g) + 2{O_2}(g)\rightleftharpoons C{O_2}(g) + 2{H_2}O(l)\)

(h) \(CuS{O_4} \times 5{H_2}O(s)\rightleftharpoons CuS{O_4}(s) + 5{H_2}O(g)\)

Complete the changes in concentrations (or pressure, if requested) for each of the following reactions.
See all solutions

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